A 90.0-mL sample of 1.00 M NaOH is mixed with 45.0 mL of 1.00 M H_2SO_4 in a lar

Question

A 90.0-mL sample of 1.00 M NaOH is mixed with 45.0 mL of 1.00 M H_2SO_4 in a large Styrofoam coffe cup; the cup is fitted with a lid through which passes calibrated thermometer.The temperature of each solution before mixing is 21.9 degree C. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.7 degree C .Assume that the density of the mixed solutions is 1.00 g/mL, that the specific heat of the mixed solutions 4.18 J/(g. degree C), and that no heat is lost to the surroundings. with a balanced chemical equation for the reaction that takes place in the Styrofoam cup. Is any NaOH or H_2^SO_4 left in the Styrofoam cup when the reaction is over? Calculate the enthalpy change per mole of H_2^SO_4 in the reaction.

Explanation / Answer

the 1st two questions are rightly solved so i am solving the last 3rd one...'

there are 45 millimoles of H2SO4

Total mass of the system = vtotal x density = (90+45)x1 =135 gram

H = msT = 135x 4.18x(30.7-21.9 ) =4965.84 joules for 45 millimoles

So for 1 mole of H2SO4 ,   H = (4965.84)/45x (1000) = 110352 joules per mole = 110.352kj/mol

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